tert-Butyllithium

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tert-Butyllithium
200px
Skeletal formula of tert-butyllithium with all implicit hydrogens shown, and partial charges added
Names
Preferred IUPAC name
tert-Butyllithium[citation needed]
Identifiers
594-19-4 YesY
3587204
ChemSpider 10254347 YesY
EC Number 209-831-5
Jmol 3D model Interactive image
PubChem 638178
UN number 3394
  • InChI=1S/C4H9.Li/c1-4(2)3;/h1-3H3; YesY
    Key: BKDLGMUIXWPYGD-UHFFFAOYSA-N YesY
  • [Li]C(C)(C)C
Properties
LiC
4H
9
Molar mass 64.055 g mol−1
Appearance Colorless solid
Density 660 mg cm−3
Boiling point 36 to 40 °C (97 to 104 °F; 309 to 313 K)
Reacts
Acidity (pKa) 53
Vapor pressure {{{value}}}
Related compounds
Related compounds
 n-Butyllithium

sec-Butyllithium
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
YesY verify (what is YesYN ?)
Infobox references

tert-Butyllithium is a chemical compound with the formula (CH3)3CLi. As an organolithium compound, it has applications in organic synthesis since it is a strong base, capable of deprotonating many carbon acids, including benzene. tert-Butyllithium is available commercially as hydrocarbon solutions; it is not usually prepared in the laboratory. Its synthesis was first reported by R. B. Woodward in 1941.[1]

Structure and bonding

Like other organolithium compounds, tert-butyllithium is a cluster. Whereas n-butyllithium exists both as a hexamer and a tetramer, tert-Butyllithium exists as tetramer with a cubane structure. Bonding in organolithium clusters involves sigma delocalization and significant Li---Li bonding.[2]

The lithium–carbon bond in tert-butyllithium is highly polarized, having about 40 percent ionic character. The molecule reacts like a carbanion, as is represented by these two resonance structures.[3] (Given the polarity calculations on the C–Li bond, the "real" structure of a single molecule of t-butyllithium is likely a near-average of the two resonance contributors shown, in which the central carbon atom has a ~50% partial negative charge while the lithium atom has a ~50% partial positive charge.)

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Chemical properties

Similar to n-butyllithium, tert-butyllithium can be used for the exchange of lithium with halogens and for the deprotonation of amines and activated C—H compounds.

This compound and other alkyllithium compounds are known to react with ether solvents; the half-life of tert-butyllithium is 60 minutes at 0 °C in diethyl ether, 40 minutes at -20 °C in tetrahydrofuran (THF),[4] and about 11 minutes at -70 °C in dimethoxyethane.[5] In this example, the reaction of tert-butyllithium with (THF) is shown:

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To minimize degradation by these solvents, reactions involving tert-butyllithium are often conducted very low temperatures in special solvents, such as the Trapp solvent mixture.

Safety

tert-Butyllithium is a pyrophoric substance, meaning that it easily catches fire on exposure to air. (A precise definition of a pyrophoric material is one "that ignite[s] spontaneously in air at or below 54.55 °C (130.19 °F)".[6]) The solvents used in common commercial preparations are themselves flammable. While it is possible to work with this compound using cannula transfer, traces of tert-butyllithium at the tip of the needle or cannula may catch fire and clog the cannula with lithium salts. While some researchers take this "pilot light" effect as a sign that the product is "fresh" and has not degraded due to time or improper storage/handling, some workers prefer to enclose the needle tip or cannula in a short glass tube, which is flushed with an inert gas and sealed at each end with septa.[7] Serious laboratory accidents involving tert-butyllithium have occurred. For example, in 2008 a staff research assistant, Sheharbano Sangji, in the lab of Patrick Harran[8] at the University of California, Los Angeles, died after being severely burned by a fire ignited by tert-butyllithium.[9][10][11]

Large-scale reactions may lead to runaway reactions, fires, and explosions when tert-butyllithium is mixed with ethers such as diethyl ether, tetrahydrofuran, and glymes.[citation needed] The use of hydrocarbon solvents may be preferred.

Air-free techniques are important so as to prevent this compound from reacting violently with oxygen and moisture in the air:

t-BuLi + O2 → t-BuOOLi
t-BuLi + H2O → t-BuH + LiOH

References

  1. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  2. ↑ Elschenbroich, C. ”Organometallics” (2006) Wiley-VCH: Weinheim. ISBN 978-3-527-29390-2
  3. ↑ Organometallic reagents: sources of nucleophilic carbon for alcohol synthesis. K. P. C. Vollhardt, N. E. Schore: Organic Chemistry : Structure And Function. 3rd edition, 1999, §8.7.
  4. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  5. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  6. ↑ SEMI, standard F6-92, Guide for Secondary Containment of Hazardous Gas Piping Systems, as cited by ChemiCool.com
  7. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  8. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  9. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  10. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  11. ↑ Los Angeles Times, 2009-03-01
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